One scale for electro negativity is based on the concept that the electro negativity of any atom is proportional to the ionization energy of the atom minus its electron affinity: electro negativity = k(IE - EA), where k is a proportionality constant.
(a) How does this definition explain why the electro negativity of F is greater than that of Cl even though Cl has the greater electron affinity?
(b) Why are both ionization energy and electron affinity relevant to the notion of electro negativity?
(c) By using data in Chapter 7, determine the value of k that would lead to an electro negativity of 4.0 for F under this definition.
(d) Use your result from part (c) to determine the electro negativities of Cl and O using this scale. Do these values follow the trend shown in Figure 8.7?

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20-2.9 Electronegativity 1.5-1.9 values have no units 15 21 40 с 130 3.5 B 25 1.5 P 25 18 21 08 10 1 15 16 08 10 12 24 28 2.5 1.8 199 20 22 16 16 18 20 118 19 22 22 22 2 P 17 1819 21 07 09 13 15 17 1 22 07 0910 13 15 1A 2A3 AB 5B 63 15 1B 2B 3A 4A 5A 6A 7A в Increasing electronegativity